Notes for Ionic Bonding
Name:_________________________________
Valence electrons: ______________________________________________________________
Lewis dot structure (electron dot configuration)
–Shows _____________________ as a series of dots surrounding an atomic symbol
–Place one dot around at a time before you double up
–Maximum of __________dots
Paired valence electrons
–Relatively _____________
–Resistant to change
–Don’t form chemical bonds
–Called _____________________________
Unpaired valence electrons
–Have a _________________ tendency to participate in chemical bonding
Atoms tend to form chemical bonds so that they each have 8 electrons (in pairs) in their valence
shells (______________ rule)
–This is similar to electron configuration of a ________________
The Octet Rule
•The octet rule says:
–Atoms tend to gain or lose electrons in order to have _________ valence electrons.
Ions and Lewis Dot Structures
•Find the number of _____________________
•Following the octet rule, find how many electrons will be gained or lost for each atom to
become an ion.
•Combine the ions to form _____________________________
Practice
•Combine the following atoms to form ionic compounds (show Lewis dot structures).
•Na Cl
•Mg F2
•Na2 O
Electrons occupy ______________shell first
–Exposed electrons in ____________________ responsible for bonding
Chemical bond
–Force of ____________________ between atoms that holds them together
 Ion : an atom having _______________________________ charge
•Cation
–An ion where electrons are __________________
–Has a __________ charge
–
Na1+ → Na+
•Electron dots for cations
–Metals will have __________ valence electrons
–These will come off
–Forming ________________ ions
•Anion
–An ion where electrons are ________________
–Ion has an overall ______________ charge
–Cl1- → Cl-
•Electron dots for anions
–Non-metals will have _____________ valence electrons
–They will ___________ electrons to fill outer shell
–Forming __________________ ions
•Ionization Energy
–The amount of energy needed to ___________ an electron from an atom
–The closer the electron is to the _________________, the harder it is to remove
•Ionic bond
•Transfer of electrons
•Formation of cations and anions
•__________________________ hold ions together
•Ionic compounds
–Are highly __________________ compounds
•each anion actually attracts several ________________
•These attract several more anions
•A network of ions forms _____________________
•Ionic compounds
•Consist of elements found on ________________ sides of the periodic table
•Positive and negative charges must _________________ (Oxidation numbers)
•When melted or ______________________, they carry an electrical charge
Criss-cross method
• Examples:
•
Mg
Cl
•
Na
S
•
Al
Br
•
Ca
N
•
Ba
P